Final answer:
The net ionic equation for the reaction of MgSO₄ with HCl would normally show magnesium ions reacting with chloride ions and hydrogen ions reacting with sulfate ions. However, since all products remain dissolved and there's no chemical change, there is no net ionic equation in this case.
Step-by-step explanation:
The net ionic equation for the reaction between MgSO₄ and HCl is as follows:
- Mg²⁺ (aq) + SO₄²⁻(aq) are the ions from MgSO₄ in an aqueous solution.
- H⁺ (aq) + Cl⁻ (aq) are the ions from HCl.
When MgSO₄ reacts with HCl in an aqueous solution, the sulfate ion (SO₄²⁻) reacts with two hydrogen ions (H⁺) to form hydrogen sulfate (HSO₄⁻), and the magnesium ion (Mg²⁺) pairs with two chloride ions (Cl⁻) to form magnesium chloride (MgCl₂).
So, the products of the reaction will be magnesium chloride and hydrogen sulfate, which remain in the solution. Therefore, the net ionic equation of this reaction could be simplified by excluding any spectator ions that do not participate in the actual chemical change. However, the provided input seems to contain a typo. Assuming it is a typical reaction between MgSO₄ and HCl, the net ionic equation would be:
Mg²⁺ (aq) + 2Cl⁻ (aq) + H⁺ (aq) + SO₄²⁻(aq) → Mg²⁺ (aq) + 2Cl⁻ (aq) + HSO₄⁻(aq)
In reality, because all the products remain in the solution as ions and there is no overall chemical change, there is no net ionic equation to be written for this specific pairing of reactants in aqueous solution.